Metallurgy and Material Selection for Mechanical Engineers A - - PowerPoint PPT Presentation

Metallurgy and Material Selection for Mechanical Engineers A Training Course Prepared and delivered by:

• Dr. A. K. Abdul Jawwad

Chapter One Structure of Metals and Alloys

• Introduction
• Physical metallurgy is concerned with

exploring and utilizing the relationships between the structures of metals and alloys and engineering properties.

• Engineers are may be interested in

several types of properties such as; physical, chemical, electrical and mechanical properties. In this course emphasis would be given to mechanical properties, which include:

• Strength
• Hardness
• Ductility
• Toughness and
• Percent elongation and
• Corrosion behavior.

• The properties of an engineering alloy

would normally determine its “performance” under certain working conditions including loading (type of load, magnitude of load, etc.) and working environment (such as working temperature, corrosiveness, etc.)

• The main factor that normally determines

these properties is the structure of the metal or alloy (at different structural levels, as will be seen later)

• In addition the structure of a certain metal
• r alloy is normally a result of both the

chemical composition and the processing route it has been through; both mechanical (such as forming, rolling, etc.) and thermal (such as welding, heat treatment, etc.).

Area of interest of physical metallurgy

Process (Mechanical & thermal) Structure Properties Performance Chemical Composition

Levels of structure

• Structure can be defined as “

Arrangement of internal building units”.

• In general there are four levels of structure

as follows:

• Sub-atomic level: this level represents

the arrangement of electrons, neutrons and protons within individual atoms.

• Atomic level: this level represents the

arrangement of atoms within special building units known as unit cells “Crystal or lattice structure”.

• Microscopic level: this level is concerned with

structural features which can be viewed by the aid of a microscope (either optical or electron microscope), “Microstructure”

• Macroscopic level: this level is concerned

with structural features which can be viewed by the naked eye or by the aid of low magnification microscope (normally below x25), “Macrostructure”

Nature of metallic bonding

Schematic illustration of metallic bonding.

• Good thermal conductivity
• Good electrical conductivity
• Normally fail in a ductile manner and show

some permanent (plastic) deformation before fracture.

Crystal structure

In a crystalline or polycrystalline solid solidification proceeds by:

• The formation of solid nuclei “crystals or

grains” at various positions with random

• rientation

• Growth of the small nuclei by the

successive addition of atoms from the surrounding liquid

• Upon completion of solidification the

crystals or grains impinge on each other forming what is known as “grain boundaries”

Crystal structure or lattice structure refers to “ arrangement of atoms in a three dimensional repetitive array over long atomic distances inside a crystal”. These three dimensional building units are known as “unit cells”

Main types of crystal structure in metals

Face-Centered-Cubic (FCC) crystal structure

• In this type of lattice structure the unit cell

has a cubic geometry with atoms located

• n the corners of this cubic cell and on the

centers of all the six cube faces.

• Typical metals having this lattice structure

include gold, silver, copper, nickel, aluminum and lead.

• The edge cube (a) known as “lattice

parameter” and the atomic radius (R) are related through the relationship:

2 2R a =

• In an FCC unit a total of four atoms is

contained within each unit cell (one eighth

• f the eight atoms on the corners plus one

half of the six atoms on the faces).

• The coordination number (number of

nearest neighbors or touching atoms) in the FCC unit cell is equal to 12 The atomic packing factor (APF) is equal to 0.74, where:

• APF = (volume of atoms in the unit

cell)/(total unit cell volume)

Body-Centered-Cubic (BCC) crystal structure

In BCC crystal structure, eight atoms

• ccupy cube corners in addition to one

atom occupying the center of the cube. Typical metals having this lattice structure include iron, chromium, molybdenum and tungsten. Relevant information to the BCC structure are:

• Coordination number = 8
• APF = 0.68

Hexagonal Close-Packed (HCP) crystal structure

• In the HCP crystal structure, the top and

bottom faces of the unit cell consist of six atoms that form regular hexagons and surround a single atom in the center. Another plane situated between the top and bottom plane provide extra three atoms

• The coordination number and APF for the

HCP unit cell are the same as those of the FCC, i.e., 12 and 0.74, respectively.

• HCP unit cell has two lattice parameters;

“a & c” representing the short and long unit cell dimensions, respectively. Typical metal having this lattice structure include; magnesium, titanium and zinc.

Crystallographic directions

• A crystallographic direction is defined as

“a line between two lattice points or a vector “

• Three directional indices of

crystallographic directions can be determined as follows:

• A vector of convenient length is

positioned such that it passes through the origin of the coordinate system. In case the vector does not pass through the origin it can be translated throughout the crystal lattice without alteration if parallelism is maintained.

• The length of the vector projection on

each of the three axes is determined in terms of lattice parameters (a, b and c).

• These numbers are multiplied or divided

by a common factor to reduce them to the smallest integer values.

• The three indices, not separated by

commas, are enclosed in square brackets, thus [u v w]. the u, v, and w values represent the x, y and z projections, respectively.

• Negative coordinates are represented by a

bar over the particular index (indices). The [100],[110], and [111] directions within a unit cell

Crystallographic planes

• Crystallographic planes (except in the

hexagonal unit cell) are represented by three Miller indices as (h k l).

• Any two planes parallel to each other are

equivalent and have identical Miller indices.

• Crystallographic planes indices can be

determined as follows:

• If the plane passes through the selected origin,

either another parallel plane must be constructed or a new origin must be established at another unit cell corner.

• At this point the plane either intersects or

parallels each of the three axes. The length of the planar intersect for each axis is determined in terms of the lattice parameters (a, b and c). A plane that parallels an axis is considered to have infinite intersect

• The reciprocals of these intersects are

taken.

• If necessary, these three numbers

(indices) are reduced to the smallest integer values.

• The integer indices, not separated by

commas, are enclosed within parentheses such as (h k l).

Representation of a series of (a) (001), (b) (110), and (c) (111) crystallographic planes

Imperfections in solids

• A defect-free solid is considered to be an

idealized condition which does not exist in reality.

• All solids contain large numbers of defects
• r imperfections.
• As a matter of fact many properties of

metallic materials are greatly sensitive to this deviation from the idealized condition not necessarily adversely.

• A crystalline defect or imperfection can be

thought of as “A lattice irregularity having one or more of its dimensions

• n the order of an atomic diameter”.
• Classification of crystalline defects is

based upon dimensionality as follows:

Point defects

• This category contain two major types of

defects

– Vacancy or vacant lattice site, one normally

• ccupied from which an atom is missing.

– Self- interstitial is an atom from the crystal that is crowded into an interstitial site (a small void space that under ordinary conditions is not occupied)

Two-dimensional representation of vacancy and a self-interstitial

Linear defects

• The main type of linear defects is the

presence of “dislocations” within the crystal.

• Dislocations are “linear or one-

dimensional defects around which some of the atoms are misaligned”

• There are two types of dislocations:

Edge dislocations

• These are linear defects which center

around the line that is defined along the end of an extra half-plane (dislocation line)

Screw dislocations

This type of dislocation can be thought of as being formed by a shear stress applied to produce the distortion ;

• The upper front region of the crystal is

shifted one atomic distance to the right relative to the bottom portion

• Dislocations are considered to play a

major roll during the phase of plastic deformation.

Interfacial defects

• These contain three major types:
• External surfaces
• Grain boundaries
• Twin boundaries. Twin boundaries are

special type of grain boundaries across which there is a specific mirror lattice symmetry

• Twin boundaries form as a result of

mechanical forming (mechanical twins) and/or during heat treatment (annealing twins).

Chapter Two The Formation of Alloys

• Even though pure metals have some

appealing properties such as high electrical and thermal conductivities, their mechanical properties generally are weak. Thus alloying is carried out to either enhance existing properties or to introduce some new properties such as corrosion resistance.

• Main requirement: complete solubility in

the liquid state, i.e. the two metals are mutually soluble in each other when in the liquid state.

• Upon solidification there are three possible

scenarios:

• Solubility is completely lost in the solid

state, therefore, the liquid solidifies as separate particles of two pure metals

• Solubility is completely or partially retained

in the solid state resulting in a single solid solution (SS) or a mixture of two solid solutions, respectively

• As solidification proceeds the two metals

give rise to the formation of what is known as “intermediate phase” or “intermetallic compound”.

• Each of the three types mentioned above

resulting from solidification is referred to as a “phase”.

• Phase can be defined as “ A single

homogeneous substance”.

• In a binary solid no more that two phases

can co-exist:

• Two pure metals
• A single solid solution
• A mixture of two solid
• solutions
• A single intermediate phase
• A mixture of two intermediate phases
• A solid solution and an intermediate

phase and so on

Solid solutions

• A solid solution is formed when two metals

which are mutually soluble in each other in the liquid state remain completely or partially soluble in each other in the solid state.

• There are two types of solid solutions

Interstitial solid solutions

• This type of solid solution can be formed

when the atoms of the added element (solute) are very small compared to those

• f the parent metal (solvent), thus

enabling them to fit into the interstices or interstitial sites of the solvent metal

• Interstitial solid solutions can form not only

as a result of solidification but also when the parent metal is in the solid state.

• A common example is plain carbon steel,

which is basically an interstitial solid solution of carbon into iron

Substitutional solid solutions

• In this type of solid solution the atoms of

the solvent are replaced by atoms of the solute metal in the lattice sites.

• Substitutional solid solutions can be either
• rdered or disordered.
• There exist some preferred conditions for

substitutional solid solutions to occur:

– Size factor (the difference in atomic radii should be less than 14 %) – Electrochemical properties should be similar (the two metal should be in close proximity in the periodic table) – The two metal having the same crystal structure (FCC into FCC and so on)

Intermediate phases

• In contrast to solid solutions intermediate

phases result when the two metals have divergent electrochemical properties, in which case a strongly metallic element such as magnesium would combine with weakly metallic element such as tin forming an intermetallic substance Mg2Sn

• Phases between the two extremes of solid

solution and intermetallic compounds are termed intermediate phases having graded properties depending on the degree of association.

• Intermediate phases have several types

including

Intermetallic compounds

• These are phases in which laws of

chemical valency are apparently obeyed such as in Mg2Sn, Mg2Pb and Mg3Bi

Electron compounds

• In these compounds there is a fixed ratio

between the number of total valence bonds of all atoms and the total number

• f atoms. According to this ratio three

types of structures exist:

– β structures (ratio of 3/2 or 21/14) such as in CuZn, Cu3Al and Ag3Al.

– γ structures (ratio of 21/13) such as in Cu5Zn8, Cu31Sn8 and Ag5Al3. – ε structures (ratio of 7/4 or 21/12) such as in CuZn3, Cu3Sn and AgCd3.

Size factor compounds

• These are intermediate phases in which

compositions and crystal structures arrange themselves in such a way as to allow the constituent atoms to pack themselves closely together.

• These include MgNi2, MgCu2, TiCr2 and

different types of metal carbides

Strengthening mechanisms in alloys

Solid solution strengthening

• In substitutional solid solutions, large

solute atoms can occupy sites where the lattice is being stretched, while small solute atoms can occupy sites where the lattice is compressed.

• This decreases the lattice distortion and

reduces the energy level and, hence impeding the movement of dislocations.

• In interstitial solid solutions, solute atoms

would normally occupy sites where the lattice is being stretched and having similar effect on movement of dislocations.

Dispersion strengthening

• The presence of small particles in the

microstructure can impede the movement

• f dislocations provided that the particles

are stronger than the matrix in which they are embedded

• The degree of strengthening depends on:

– The particle size – Inter-particle spacing – Type of particles (hardness); and – The volume fraction (content) of the strengthening particles

Chapter Three

Thermal Equilibrium Diagrams (Phase Diagrams)

• Thermal equilibrium diagrams are “charts

showing the relationships between chemical composition, temperature and phases present”.

• Equilibrium means a state of balance,

i.e., the system (alloy) is allowed enough time to reach this state of equilibrium normally through slow cooling rates.

• Several types of binary phase diagrams

exist depending on the relation ship between the two components (alloying elements) such as solubility limits, electronegativity properties, atomic size, etc.

Binary isomorphous system

• The term isomorphous indicates complete

solubility in both the liquid and solid states

• The reason for this complete solubility in

the solid state comes as a result from the fact that both Ni and Cu have the same crystal structure (FCC), almost identical atomic sizes and electronegativities.

• In this diagram several features can be

noticed

– The temperature is plotted on the vertical axis while the composition (in terms of solute percentage) is plotted on the horizontal axis.

• There exist three main areas in the

diagram (known as phase fields) of liquid, α + liquid and α, where liquid is a homogenous liquid solution of both Cu and Ni and α is a homogenous solid solution of both Cu and Ni with an FCC crystal structure

• The line over which all compositions are in

the liquid state is termed as the “Liquidus”

• The line below which all compositions are

in the solid state is termed as the “Solidus”

• On the event of a vertical line crossing a

sloping line on a phase field, the number

• f phases changes by one (either increase
• r decrease).
• A phase which does not have a phase

field but appears in a two-phase field is either a pure metal or an intermediate phase.

Three kinds of information can be readily

• btained from binary phase diagrams:
• Phases that are present
• Composition of these phases
• Percentages or fractions of

Phases present

• Establishing what phases are present is

quite simple; one has just to locate the temperature-composition point on the diagram and note the phase(s) with which the corresponding phase field is labeled.

• For example an alloy of composition 60%

Ni and 40% Cu at 1100 °C would be located at point A and consist of a single solid solution α.

• On the other hand an alloy of composition

35% Ni and 65% Cu at 1250 °C would be located at point B and consist L + α phases.

Determination of phase compositions

• The composition of the phases present

can be determined through the following steps:

• The temperature-composition point has to

be located.

• If this point falls within a single-phase field

then the composition of this phase is the same as the original alloy.

• If this point falls within a two-phase field a

horizontal line (known as a tie line) is constructed from this point extending both sides until it intersects the two phase boundaries.

• The two intersect on both phase boundaries

are noted and perpendiculars (vertical lines) are dropped on the horizontal (composition) axis from which compositions of the respective phases are determined

• Determination of phase compositions for

an alloy containing 35% Ni and 65% Cu at 1250 °C is shown point B indicating a liquid composition (CL) of 31.5% Ni and an α composition (Cα) of 42.5% Ni.

Determination of phase amounts

• The determination of phase amounts is

quite similar and depend on the determination of phase composition.

• This is done by applying the “Lever rule”

Wt%

phase B Wt% phase A Composition of phase B Composition

• f phase A

Overall composition

• In order to keep the balance around the
• verall composition then the following

condition applies: (Wt% of phase A)x(Composition of phase A

• Overall composition)

= (Wt% of phase B)x (Overall composition - Composition of phase B)

• For the alloy of point B this results in the

following:

• Or by subtracting compositions,

S R S WL + =

% 68 68 . 5 . 31 5 . 42 35 5 . 42 = = − − = − − =

l

• L

C C C C W

α α

• The weight percentage of α phase can be

determined in the same manner

% 32 32 . 5 . 31 5 . 42 5 . 31 35 = = − − = − − = + =

L L

• C

C C C S R R W

α α

Determination of microstructural developments under equilibrium and non- equilibrium conditions

• The development of microstructure can be

determined by following a solidification path of an alloy of a certain chemical composition.

• The previous example of an alloy with over

all composition of 35% Ni and 65% Cu will be considered